By Adnan A. Multiple Choice [Fill in the Blank]
1. Tin is actually coated with a thin layer of tin.
a. Steel b. Iron c.Chromium d. Shamwow
2. is the process in which iron is covered with a protective layer of Zinc.
a. Steel b.Protection c. Galvanizing d. Cathodic Protection
3. , is and example of Corrosion.
a. Rusting b. Decomposition c. Corrosion d. Separation Short Answers
1. Why would metal parts of cars corrode faster in the Atlantic provinces than the metal parts of cars elsewhere?
2. Corrosion isn't all bad. Give one example of corrosion that can be used.
ANSWER KEY: Multiple Choice
1. A
2. C
3. A
Short Answers
1. Metal parts would corrode faster in the Atlantic provinces because of the moister in the air because Atlantic provinces are near large bodies of water as compared to provinces that are not. The water in the Air accelerates the rusting process.
2. Artists can use rusting and corrosion in their favor because it gives a good colour to the material.
_ By Xinli Tu
MULTIPLE CHOICE
1. What is the meaning of corrosion? a) Characteristic of metals which indicate that they are reddish-brown in colour b) Spontaneous redox reactions of materials with substances in the environment c) The process in which metals are worn down from overuse d) The process that is used to prevent precipitation
2. For rusting to occur, _ is needed. (Fill in the blank) a) Carbon dioxide b) Carbonic acid c) Rainwater d) Tap water e) Two of the above f) None of the above
3. The process of attaching a more reactive metal to an iron object that will act as an anode is called a) Cathodic protection b) Erosion protection c) Sacrificial protection d) Photosynthesis
SHORT ANSWERS
4. Not all metals corrode to the same extent as iron. Give an example where the corrosion of a metal is beneficial and explain why it is beneficial.
5. What are two ways in which the galvanizing process helps zinc protect iron?
ANSWERS1. B2. C3. A4. Metals such as aluminum corrode in air to form a surface coating of a metal oxide that adheres to the metal surface and forms a protective layer that prevents the metal from further corrosion.5. First of all, the zinc acts as a protective layer which means it will not be exposed to air and water. Secondly, even if this zinc layer is scratched or broken, it still acts as protection because zinc is more easily oxidized than iron. Thus, zinc becomes the anode instead of iron in the galvanic cell so iron does not corrode until all the zinc has reacted.
BY JACKIELYN JABSON Multiple Choice Questions 1. In preventing corrosion, aluminum acts as…a. A protective layer
b. sacrificial anode
c. oxidizing agent
d. All of the above
2. In cathodic protection, what type of metal is attached to the iron object?a. Alloy
b. Tin
c. A more reactive metal
d. Less reactive metal
e. None of the above
3. Corrosion is…a.a spontaneous redox reaction between liquids and solidsb. a non-spontaneous redox reaction between materials and substances in the environment c. Caused by the spontaneous formation of galvanic cells on the surface of metals
Short Answers: 4. In cathodic protection, what is the consequence of using a metal that is less reactive than iron? Provide an example.
5. If a piece of iron was placed on the moon, at what rate would the piece of iron rust? Explain.
ANSWERS: Multiple Choice 1. b
2. c
3. c
Short Answer: 4. Using a metal that is less reactive than iron can cause iron to corrode faster when it is exposed to oxygen due to its contact with the less reactive metal. A tin can is a steel can coated with a thin layer of tin. While the tin layer remains intact, it provides protection against rusting. If layer is broken or scratched, the iron in the steel corrodes faster in contact with the tin that the iron would on its own. Tin is less reactive than iron, thus tin acts as a cathode and iron acts as the anode. 5.The moon’s conditions would prevent the corrosion of the piece of iron, thus it will not rust. Corrosion is a spontaneous redox reaction between materials and substances in the environment. Iron corrodes to due to its interaction with oxygen, water (in rain form), and carbon dioxide. Carbon dioxide in the air reacts with rainwater to form carbonic acid. Carbonic acid is an electrolyte for the corrosion process. Oxygen is the oxidizing agent. The moon does not have these factors, therefore corrosion cannot occur.
By Yasar Chowdhury Multiple Choice
1. During the rusting process, what material is used as the cathode?
a) Iron
b) Any impurity deposited on the iron
c) Oxygen
d) Water
2. What material is used to coat iron in the galvanizing process?
a) Copper
b) Tin
c) Zinc
d) None of the above
3. What is the process of attaching a more reactive metal to an iron object in order to prevent corrosion?3
a) Sacrificial anode
b) Galvanization
c) Cathodic protection
d) Electron Beam Coating
Short Answer
1. A ‘tin’ can is a steel can coated with the less reactive metal, tin. When the can is scratched or punctured, the steel corrodes faster than if it were directly exposed to air. How can coating an iron object with tin, a less reactive metal, cause the object to corrode at a faster rate?
2. How does mixing metals into an alloy help it resist corrosion?
Answers:
Multiple Choice: 1.b) 2.c) 3.c)
Short answer:
1. Because tin is less reactive, it acts as a cathode in each miniature galvanic cell on the surface of the can. Iron acts as an anode, as it normally would in the rusting process. The large area of available cathodes provided by the tin causes more reactions to occur.
2. The overall resistance to corrosion increase with the addition of corrosive resistant materials.
By: Andrew Vyravipillai
MULTIPLE CHOICE
1. How do objects experience corrosion?
a) through the process of galvanziation
b) if they are not kept cool, dry and clean
c) through oxidation with the external environment
d) two of the above
e) none of the above
2. A sacrificial anode is:
a) a highly reactive element
b) a metal which oxidizes more easily than others, and is destroyed to protect the other object
c) an good conductor of electricity which is a strong oxidizing agent
d) only B
e) A and B
f) A and C
g) all of the above
3. What is one of the best metals to aide in the formation of an alloy
a) stainless steel
b) chromium
c) iron
d) zinc
SHORT ANSWER
4. How is the corrosion of iron different from other metals?
5. What is the difference between galvanization and cathodic protection?
Answer Key:
1. D
2. D
3. A
4. Not all metals corrode to the same extent as iron, many metals corrode in air to form a surface coating of metal oxide which adheres to the metal surface and forms a protective layer that prevents further corrosion. In contrast, rust easily flakes off from the surface of iron and provides little to no protection against further corrosion.
5. The difference between galvanization and cathodic protection is that galvanizing refers to cover the iron completely with a protective layer of zinc for protection, however in cathodic protection it does not completely cover the metal, since it is the sacrificial anode, it also must be replaced periodically.__
Udari Premachandra
Multiple Choice and Short Answer Questions
1. What type of reaction is rusting?
a) Spontaneous
b) Non-spontaneous
c) Redox
d) A and C
2. What percentage of iron and steel is produced to replace objects that have been damaged by corrosion?
a) 40-45%
b) 2-5%
c) 20-25%
d) 60-75%
3. What is the green layer formed by the corrosion of a copper roof called?
a) Platina
b) Patina
c) Plateau
d) Enamel
4. Explain why metal plates, pots and pans do not corrode?
5. Why is stainless steel often used for cutlery, taps and other small applications?
Answers
Corrosion:
D
C
B
Metal plates, pots and pans do not corrode because there is an enamel coating to protect them. Enamel is a shiny, hard and very nonreactive type of glass that can be melted onto a metal surface.
Stainless steel is often used because stainless steel is an alloy for iron and is also more resistant to corrosion than pure iron.
Abinethaa Paramasivam Short Answers: 1) Describe one way how can corrosion can be used in a no harmful way. Corrosion can be useful when people consider the green layer formed by corrosion of a copper roof attractive. The layer, called patina is formed and protects the copper beneath it from further corrosion.
2) Explain the process of rusting. Rust is composed of hydrated iron (III) oxide is made of small galvanic cells in which electrochemical reactions form rust. In each, the iron is the anode and the cathode is the inert. Water in form of rain required for rusting to occur in which the CO2 in air reacts with rainwater to form carbonic acid. It dissociates into ions and thus carbonic acid is electrolyte for corrosion process.
Multiple Choices: 1) Corrosion of iron can be prevented by: - Attaching a more reactive metal to iron object - Attaching less reactive metal to iron object - Paint the iron object - Form an alloy with different metal than iron Answer: B
2) The process galvanizing is when: a) Process of covering zinc with protective layer of zinc b) Process of covering zinc with protective layer of iron c) Metal oxidizes more easily that iron and destroyed to protect an object d) Process of covering iron with protective layer of zinc Answer: D
Khevna Patel
Multiple choice:
1. In the corrosion of iron, which of the following is the anode? Which is the cathode?
a) Iron, any impurity deposited on the iron
b) Any impurity deposited on the iron, iron
c) Iron, oxygen
d) None of the above
2. Corrosion can be prevented by
a) Painting the object
b) Spraying the object with water
c) Avoiding galvanization
d) Cathodic protection
e) None of the above
f) Both a and d
3. Galvanizing is a process in which
a) Iron is protected from rusting
b) Iron is covered with a protective layer of potassium
c) Iron protects other metals from rusting
d) Iron is covered with a protective layer of zinc
e) Two of the above
f) All of the above
Short Answer:
1. Describe the process of cathodic protection, and why it must be done a certain way.
2. What is a major drawback to cathodic protection?
ANSWERS:
Multiple choice
A
F
E
Short Answer
Cathodic protection is a process by which an iron object is protected from oxygen in the air, and is therefore protected from corroding. A more reactive metal is attached to the iron object, acting as an anode and prevents the iron from reacting with oxygen until that metal has not fully reacted (corroded). The metal must be more reactive than iron because if it is less reactive and is scratched, it can speed up the corrosion of iron. A less reactive metal covering will act as a cathode and allow the oxidization of iron to happen faster.
The protective layer on the iron does not completely cover the iron since it is slowly being destroyed by oxidization. Therefore, the protective layer must be replaced periodically to continuously protect the iron.
Multiple Choice [Fill in the Blank]
1. Tin is actually coated with a thin layer of tin.
a. Steel b. Iron c.Chromium d. Shamwow
2. is the process in which iron is covered with a protective layer of Zinc.
a. Steel b.Protection c. Galvanizing d. Cathodic Protection
3. , is and example of Corrosion.
a. Rusting b. Decomposition c. Corrosion d. Separation
Short Answers
1. Why would metal parts of cars corrode faster in the Atlantic provinces than the metal parts of cars elsewhere?
2. Corrosion isn't all bad. Give one example of corrosion that can be used.
ANSWER KEY:
Multiple Choice
1. A
2. C
3. A
Short Answers
1. Metal parts would corrode faster in the Atlantic provinces because of the moister in the air because Atlantic provinces are near large bodies of water as compared to provinces that are not. The water in the Air accelerates the rusting process.
2. Artists can use rusting and corrosion in their favor because it gives a good colour to the material.
_
By Xinli Tu
MULTIPLE CHOICE
1. What is the meaning of corrosion?
a) Characteristic of metals which indicate that they are reddish-brown in colour
b) Spontaneous redox reactions of materials with substances in the environment
c) The process in which metals are worn down from overuse
d) The process that is used to prevent precipitation
2. For rusting to occur, _ is needed. (Fill in the blank)
a) Carbon dioxide
b) Carbonic acid
c) Rainwater
d) Tap water
e) Two of the above
f) None of the above
3. The process of attaching a more reactive metal to an iron object that will act as an anode is called
a) Cathodic protection
b) Erosion protection
c) Sacrificial protection
d) Photosynthesis
SHORT ANSWERS
4. Not all metals corrode to the same extent as iron. Give an example where the corrosion of a metal is beneficial and explain why it is beneficial.
5. What are two ways in which the galvanizing process helps zinc protect iron?
ANSWERS1. B2. C3. A4. Metals such as aluminum corrode in air to form a surface coating of a metal oxide that adheres to the metal surface and forms a protective layer that prevents the metal from further corrosion.5. First of all, the zinc acts as a protective layer which means it will not be exposed to air and water. Secondly, even if this zinc layer is scratched or broken, it still acts as protection because zinc is more easily oxidized than iron. Thus, zinc becomes the anode instead of iron in the galvanic cell so iron does not corrode until all the zinc has reacted.
BY JACKIELYN JABSON
Multiple Choice Questions
1. In preventing corrosion, aluminum acts as…a. A protective layer
b. sacrificial anode
c. oxidizing agent
d. All of the above
2. In cathodic protection, what type of metal is attached to the iron object?a. Alloy
b. Tin
c. A more reactive metal
d. Less reactive metal
e. None of the above
3. Corrosion is…a.a spontaneous redox reaction between liquids and solidsb. a non-spontaneous redox reaction between materials and substances in the environment
c. Caused by the spontaneous formation of galvanic cells on the surface of metals
Short Answers:
4. In cathodic protection, what is the consequence of using a metal that is less reactive than iron? Provide an example.
5. If a piece of iron was placed on the moon, at what rate would the piece of iron rust? Explain.
ANSWERS:
Multiple Choice
1. b
2. c
3. c
Short Answer:
4. Using a metal that is less reactive than iron can cause iron to corrode faster when it is exposed to oxygen due to its contact with the less reactive metal. A tin can is a steel can coated with a thin layer of tin. While the tin layer remains intact, it provides protection against rusting. If layer is broken or scratched, the iron in the steel corrodes faster in contact with the tin that the iron would on its own. Tin is less reactive than iron, thus tin acts as a cathode and iron acts as the anode.
5. The moon’s conditions would prevent the corrosion of the piece of iron, thus it will not rust. Corrosion is a spontaneous redox reaction between materials and substances in the environment. Iron corrodes to due to its interaction with oxygen, water (in rain form), and carbon dioxide. Carbon dioxide in the air reacts with rainwater to form carbonic acid. Carbonic acid is an electrolyte for the corrosion process. Oxygen is the oxidizing agent. The moon does not have these factors, therefore corrosion cannot occur.
By Yasar Chowdhury
Multiple Choice
1. During the rusting process, what material is used as the cathode?
a) Iron
b) Any impurity deposited on the iron
c) Oxygen
d) Water
2. What material is used to coat iron in the galvanizing process?
a) Copper
b) Tin
c) Zinc
d) None of the above
3. What is the process of attaching a more reactive metal to an iron object in order to prevent corrosion?3
a) Sacrificial anode
b) Galvanization
c) Cathodic protection
d) Electron Beam Coating
Short Answer
1. A ‘tin’ can is a steel can coated with the less reactive metal, tin. When the can is scratched or punctured, the steel corrodes faster than if it were directly exposed to air. How can coating an iron object with tin, a less reactive metal, cause the object to corrode at a faster rate?
2. How does mixing metals into an alloy help it resist corrosion?
Answers:
Multiple Choice: 1.b) 2.c) 3.c)
Short answer:
1. Because tin is less reactive, it acts as a cathode in each miniature galvanic cell on the surface of the can. Iron acts as an anode, as it normally would in the rusting process. The large area of available cathodes provided by the tin causes more reactions to occur.
2. The overall resistance to corrosion increase with the addition of corrosive resistant materials.
By: Andrew Vyravipillai
MULTIPLE CHOICE
1. How do objects experience corrosion?
a) through the process of galvanziation
b) if they are not kept cool, dry and clean
c) through oxidation with the external environment
d) two of the above
e) none of the above
2. A sacrificial anode is:
a) a highly reactive element
b) a metal which oxidizes more easily than others, and is destroyed to protect the other object
c) an good conductor of electricity which is a strong oxidizing agent
d) only B
e) A and B
f) A and C
g) all of the above
3. What is one of the best metals to aide in the formation of an alloy
a) stainless steel
b) chromium
c) iron
d) zinc
SHORT ANSWER
4. How is the corrosion of iron different from other metals?
5. What is the difference between galvanization and cathodic protection?
Answer Key:
1. D
2. D
3. A
4. Not all metals corrode to the same extent as iron, many metals corrode in air to form a surface coating of metal oxide which adheres to the metal surface and forms a protective layer that prevents further corrosion. In contrast, rust easily flakes off from the surface of iron and provides little to no protection against further corrosion.
5. The difference between galvanization and cathodic protection is that galvanizing refers to cover the iron completely with a protective layer of zinc for protection, however in cathodic protection it does not completely cover the metal, since it is the sacrificial anode, it also must be replaced periodically.__
Udari Premachandra
Multiple Choice and Short Answer Questions
1. What type of reaction is rusting?
a) Spontaneous
b) Non-spontaneous
c) Redox
d) A and C
2. What percentage of iron and steel is produced to replace objects that have been damaged by corrosion?
a) 40-45%
b) 2-5%
c) 20-25%
d) 60-75%
3. What is the green layer formed by the corrosion of a copper roof called?
a) Platina
b) Patina
c) Plateau
d) Enamel
4. Explain why metal plates, pots and pans do not corrode?
5. Why is stainless steel often used for cutlery, taps and other small applications?
Answers
Corrosion:
Abinethaa Paramasivam
Short Answers:
1) Describe one way how can corrosion can be used in a no harmful way.
Corrosion can be useful when people consider the green layer formed by corrosion of a copper roof attractive. The layer, called patina is formed and protects the copper beneath it from further corrosion.
2) Explain the process of rusting.
Rust is composed of hydrated iron (III) oxide is made of small galvanic cells in which electrochemical reactions form rust. In each, the iron is the anode and the cathode is the inert. Water in form of rain required for rusting to occur in which the CO2 in air reacts with rainwater to form carbonic acid. It dissociates into ions and thus carbonic acid is electrolyte for corrosion process.
Multiple Choices:
1) Corrosion of iron can be prevented by:
- Attaching a more reactive metal to iron object
- Attaching less reactive metal to iron object
- Paint the iron object
- Form an alloy with different metal than iron
Answer: B
2) The process galvanizing is when:
a) Process of covering zinc with protective layer of zinc
b) Process of covering zinc with protective layer of iron
c) Metal oxidizes more easily that iron and destroyed to protect an object
d) Process of covering iron with protective layer of zinc
Answer: D
Khevna Patel
Multiple choice:
1. In the corrosion of iron, which of the following is the anode? Which is the cathode?
a) Iron, any impurity deposited on the iron
b) Any impurity deposited on the iron, iron
c) Iron, oxygen
d) None of the above
2. Corrosion can be prevented by
a) Painting the object
b) Spraying the object with water
c) Avoiding galvanization
d) Cathodic protection
e) None of the above
f) Both a and d
3. Galvanizing is a process in which
a) Iron is protected from rusting
b) Iron is covered with a protective layer of potassium
c) Iron protects other metals from rusting
d) Iron is covered with a protective layer of zinc
e) Two of the above
f) All of the above
Short Answer:
1. Describe the process of cathodic protection, and why it must be done a certain way.
2. What is a major drawback to cathodic protection?
ANSWERS:
Multiple choice
- A
- F
- E
Short Answer